Question

Cordell bought new tires for his bicycle. As he rode his bike on the hot street, the temperature of the air in the tires increased. If the volume of the air stayed the same, what happened to the pressure inside the tires?

A. It decreased. B. It increased. C. It stayed the same. D. It was inversely proportional to the temperature

Answer 1

Answer: The answer is B. The pressure inside the tires increased.

Step-by-step explanation:

The relationship between the pressure, volume, and temperature of a gas is described by the ideal gas law, which is usually written as:

`$$PV = nRT$$`

where:

-
`\(P\)` is the pressure,

-
`\(V\)` is the volume,

-
`\(n\)` is the number of moles of gas,

-
`\(R\)` is the ideal gas constant, and

-
`\(T\)` is the temperature (in Kelvin).

In this case, the volume
`\(V\)` and the number of moles
`\(n\)` of air in the tires stay the same. The temperature
`\(T\)` is increasing. Therefore, for the equation to remain balanced, the pressure
`\(P\)` must also increase.

So, the answer is B. The pressure inside the tires increased.